## To find the normal boiling point of the solution, we can use the formula:

bp = 100 + N * kb * m

where bp is the boiling point in °C, N is the number of particles the solute dissociates into, kb is the boiling point elevation constant for the solvent (in this case, water), and m is the molality of the solution.

First, we need to calculate N, which represents the number of particles the solute dissociates into. Since it is stated that the solute is a nonvolatile solute, it does not evaporate or dissociate into ions in the solution. Therefore, N = 1.

Now, we need to find kb for water. The boiling point elevation constant, kb, for water is 0.512 °C/m.

Next, we need to calculate the molality of the solution. The molality is defined as the number of moles of solute per kilogram of solvent. In this case, we have a 0.010 m aqueous solution, which means that there are 0.010 moles of solute per kilogram of water.

Finally, we can substitute the values into the formula to find the normal boiling point:

bp = 100 + 1 * 0.512 * 0.010

= 100 + 0.00512

= 100.00512 °C

Therefore, we would expect the normal boiling point of this solution to be approximately 100.00512 °C.